Question

Given the following:

N2 + 1/2 O2 --> N2O Kc = 1.0x10^18
What is the equilibrium constant of the following reaction?
2N2O --> 2N2 + O2 Kc =

a) 2.0 x 10^-18
b) 2.0 x 10^18
c) -2.0 x 10^-18
d) -2.0 x 10^18
e) 1.0 x 10^36

Answer 1

The equilibrium constant for the reverse reaction 2N2O → 2N2 + O2 is found by taking the reciprocal and squaring the given equilibrium constant for N2 + 1/2 O2 → N2O, resulting in 1.0 x 10^-36, corresponding to option e.

Step-by-step explanation:

The equilibrium constant (Kc) for the reaction N2 + 1/2 O2 → N2O is given as 1.0 x 1018. To find the equilibrium constant for the reverse reaction, which in this case is 2N2O → 2N2 + O2, we take the reciprocal of the original Kc and square it because the coefficients of the reaction have doubled. This will give us (1 / (1.0 x 1018))2, or 1.0 x 10-36. Therefore, the equilibrium constant for the reverse reaction is 1.0 x 10-36, which corresponds to choice e.